Deduce the balanced chemical equation for the reaction between sodium and sulfur. State the electron arrangements of the reactants and product, and explain whether sulfur is oxidized or reduced.
Question
Deduce the balanced chemical equation for the reaction between sodium and sulfur. State the electron arrangements of the reactants and product, and explain whether sulfur is oxidized or reduced.
Solution
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The reaction between sodium (Na) and sulfur (S) forms sodium sulfide (Na2S). The balanced chemical equation is:
2Na + S โ Na2S
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Electron arrangements:
- Sodium (Na) has an electron configuration of [Ne]3s1. It has 1 electron in its outermost shell.
- Sulfur (S) has an electron configuration of [Ne]3s23p4. It has 6 electrons in its outermost shell.
- Sodium sulfide (Na2S) is an ionic compound. Each sodium atom donates one electron to sulfur, resulting in two sodium ions (Na+) with electron configuration of [Ne] and a sulfide ion (S2-) with electron configuration of [Ne]3s23p6.
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In this reaction, sulfur gains electrons from sodium and is therefore reduced. Sodium loses electrons and is therefore oxidized. This is a redox reaction where sodium is the reducing agent and sulfur is the oxidizing agent.
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